(b) KCl — potassium chloride, KOH — potassium hydroxide, KClO3 — potassium chlorate.
(c) KCl — ionic, KOH — ionic, KClO3 — ionic.
[ K] + [ Cl ] – → KCl
[ K] + [ O — H ] – → K OH
[ K] +
O — Cl — O
→ K ClO3
:O:
(d) KCl — binary, KOH — tertiary and basic, KClO3 — tertiary.
(e) KCl — ionic bonds only, KOH — ionic and covalent bonds, KClO3 — ionic and covalent bonds.
CHAPTER 2 SUMMARY
Make a Summary
(Page 102)
The examples of NaCl and H2O are used in the table below. The student is to include as many examples of compounds
as possible for each type of intramolecular bond.
Table 1: Summarizing Bonds and Forces
Compound
Properties
NaCl
Solid at SATP,
hard and
brittle, high
melting point,
its solution
conducts
electricity.
H 2O
Liquid at
SATP, low
boiling point.
Electron dot
diagram/ Lewis
structure
[Na]+ [Cl]–
Intramolecular
bond type
Polarity
Intermolecular
forces
Ionic
Ionic
Locked in
a regular
structure, held
by the balance
of attractive
bonds and
electrical repulsion.
H–O–H
Covalent
Polar
Hydrogen bonds.
Reflect on your Learning
(Page 102)
By the end of the chapter the student should have developed a more in-depth understanding of why atoms form
compounds, an awareness of the many different compounds that are possible, the types of forces present between
atoms in compounds, and how the forces that hold atoms together in a compound determine the chemical properties
of the compound.
CHAPTER 2 REVIEW
(Page 103)
Understanding Concepts
1. When elements that are found in the “metals” position in the periodic table react with elements that are found in the
“nonmetals” position in the periodic table, they form ionic compounds that have ionic bonds. When elements that are
found in the “nonmetals” position in the periodic table react with elements also found in the “nonmetals” position in
the periodic table, they form molecular compounds that have covalent bonds.
Copyright © 2002 Nelson Thomson Learning
Chapter 2 Chemical Bonding
45